Can you represent the reduction of perchlorate to chloride by oxidation of $N O_{2}$ $NO_2$ to nitrate anion?

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Answer 1 · 2017-05-26T15:42:22

Well, $perchlorate ion$ $"perchlorate ion"$ is reduced from $C l (V I I +)$ $Cl(VII+)$ to $C l (- I)$ $Cl(-I)$ ....

$C l O_{4}^{-} + 8 H^{+} + 8 e^{-} \to C l^{-} + 4 H_{2} O (l)$ $ClO_4^(-) + 8H^(+) + 8e^(-) rarr Cl^(-) + 4H_2O(l)$ $(i)$ $(i)$

And $N O_{2}$ $NO_2$ is oxidized, $N (I V +)$ $N(IV+)$ to $N (V +)$ $N(V+)$ :

$N O_{2} (g) + H_{2} O \to N O_{3}^{-} + 2 H^{+} + e^{-}$ $NO_2(g) +H_2O rarr NO_3^(-) +2H^(+) +e^-$ $(i i)$ $(ii)$

And so to eliminate the electrons, we take $(i) + 8 \times (i i)$ $(i) + 8xx(ii)$ :

$8 N O_{2} (g) + 4 H_{2} O + C l O_{4}^{-} \to 8 N O_{3}^{-} + 8 H^{+} + C l^{-}$ $8NO_2(g) +4H_2O+ClO_4^(-) rarr 8NO_3^(-) +8H^(+) + Cl^(-)$

Is this balanced with respect to mass and charge?

Can you represent the reduction of perchlorate to chloride by oxidation of NO2NO_2 to nitrate anion?